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Understanding Chemical Bonding Fundamentals

Learn about forming compounds, bonding types, and properties of ionic and molecular compounds. Explore how atoms interact, create bonds, and the role of valence electrons. Discover the characteristics of metals, non-metals, and diatomic molecules in this informative guide.

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Understanding Chemical Bonding Fundamentals

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  1. Forming Compounds: Bonding

  2. Bonding • When two atoms collide, valence electrons on both atoms interact. • A chemical bond is created between the atoms if the valence electrons rearrange so that the new compound has less energy than before. • The lowest energy arrangement of electrons is the same as the noble gases (8 valence electrons = happy)

  3. Ionic • Ionic compounds are made up of cations and anions • the attractive force between oppositely charge ions (+ and -) is called an ionic bond • Nearly all ionic compounds are between metal cations and non-metal anions. • A compound with a crystalline shape is formed.

  4. An atom can: • Give up electrons: forms an ion with a positive charge (cation) • Gain electrons: forms an ion with a negative charge (anion) • Share electrons: two atoms might share pairs of electrons (might share 1 pair, 2 pairs, or 3 pairs) • if 1 pair is shared= single bond • If 2 pairs are shared = double bond • If 3 pairs are shared = triple bond

  5. Metals and Non-Metals • Remember: planetary models • Metals want to give away electrons • Ex. Na has 1 valence electron to give away • Ex. Mg has 2 valence electrons to give away • Ex. Al has 3 valence electrons to give away • Non-metals want to gain electrons • Ex. O has 2 valence electrons it wants to gain • Ex. Fluorine has 1 valence electron it wants to gain

  6. Ionic Compounds: Properties • Relatively high melting points; large energy amount needed to break apart attraction forces in bond • Conduct electricity when molten or dissolved in water • Not electrical conductors in solid state

  7. Molecular • Molecular compounds are substances composed of molecules; joined by covalent bonds • When atoms share a pair of electrons they are joined by a covalent bond • Electrons move back and forth between the outer energy levels of each atom in the covalent bond. • Most molecular compounds are made up of 2 or more non-metal elements

  8. Molecular Compounds: Properties • Relatively low melting points because little energy is needed to break attractive forces in bond • Do not conduct electricity when solid or liquid or dissolved in water (aqueous, aq)

  9. Diatomic Molecule • “di” means “two” • Diatomic molecule contains two atoms • Ex. Fluorine molecule F2 • These elements either have to: • Be bonded to themselves ex. F2, Cl2, H2 Or • Be bonded to another element ex. HBr, CO

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